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Radioactive decay follows which order reaction?

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Important Questions on Chemical Kinetics

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

Which among the following reactions can be an example of pseudo first order reaction?

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The half-life period of a first-order chemical reaction is

6.93

minutes. The time required for the completion of

99 %

of the chemical reaction will be

(\log 2 = 0 .301)

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The rate constant for a first order reaction is

7 .0 \times 10^{- 4} s^{- 1} .

If initial concentration of the reactant is

0.080 M

, what is the half-life of the reaction?

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The half-life period of a first-order reaction is

15 minutes

. The amount of substance left after one hour will be

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The rate of a first-order reaction is

0.04 m o l l^{- 1} s^{- 1}

10

second and

0.03 m o l l^{- 1} s^{- 1}

20

seconds after initiation of the reaction. The half-life period of the reaction is:

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

A first-order reaction has a specific reaction rate

10^{- 2} \sec^{- 1} .

How much time will it take for

20 g

the reactant to reduce to

5 g

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

When initial concentration of a reactant is doubled in a reaction, its half-life period is not affected. The order of the reaction is:

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

A flask contains a mixture of compounds

A

and

B

. Both compounds decompose by first-order kinetics. The half-lives for

A

and

B

are

300 s

and

180 s

, respectively. If the concentrations of

A

and

B

are equal initially, the time required for the concentration of A to be four times that of

B

(in s) is :

(Use \ln 2 = 0.693)

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

Decomposition of

X

exhibits a rate constant of

0 .05 μg / year

. How many years are required for the decomposition of

5 μg

X

into

2 .5 μg

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The rate constant of the reaction

A ⟶ B

0.6 \times 10^{- 3}

mole per liter per second. If the initial concentration of A is 5 M, then the concentration of B after 20 minutes is:

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The rate constant for the first order reaction is

60 s^{- 1} .

How much time will it take to reduce the concentration of the reactant to

\frac{1}{16} t h

value?

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The half-life of the first-order reaction,

{CH}_{3} CHO (g) \to {CH}_{4} (g) + CO (g)

, if the initial pressure of

{CH}_{3} CHO (g)

80 mm

Hg

and the total pressure at the end of

20

minutes is

120 mm

Hg

, is:

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

If the rate constant for a first order reaction is

k

, the time

(t)

required for the completion of

99 %

of the reaction is given by

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

For a zero - order reaction with rate constant k, the slope of the plot reactant concentration against time is

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

A bacterial infection in an internal wound grows as

N^{'} (t) = N_{0} e x p (t)

, where the time

t

is in hours. A dose of antibiotic, taken orally, needs 1 hour to reach the wound. Once it reaches there, the bacterial population goes down as

\frac{d N}{d t} = - 5 N^{2}

. What will be the plot of

\frac{N_{0}}{N}

t

after

1

hour?

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The half-life for a zero order reaction having

0.02 M

initial concentration of reactant is

100 s

. The rate constant (in

mol L^{- 1} s^{- 1}

) for the reaction is

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The rate constant for a first order reaction is

4.606 \times 10^{- 3} s^{- 1}

. The time required to reduce

2.0 g

of the reactant to

0.2 g

is :

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The reaction

2 N_{2} O_{5} (g) \to 4 N O_{2} (g) + O_{2} (g)

follows first order kinetics. The pressure of a vessel containing only

N_{2} O_{5}

was found to increase from 50 mm Hg to 87.5 mm Hg in 30 min. The pressure exerted by the gases after 60 min. Will be (Assume temperature remains constant) :

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

N_{2} O_{5}

decomposes to

{NO}_{2}

and

O_{2}

follows the first order kinetics. After

50

minutes, the pressure inside the vessel increases from

50 mm Hg

87.5 mm Hg

. The pressure of the gaseous mixture after

100

minutes at constant temperature will be:

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

When initial concentration of the reactant is doubled, what happens to the half-life period of a zero order reaction?

Radioactive decay follows which order reaction?

Important Questions on Chemical Kinetics

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